Diborane

Aluminium forms a polymeric hydride, (AlH3)n; although unstable, Al2H6 has been isolated in solid hydrogen and is isostructural with diborane.

Similarly, oxidation of borohydride salts has been demonstrated and remains convenient for small-scale preparations.

For example, using iodine as an oxidizer:[13] Another small-scale synthesis uses potassium borohydride and phosphoric acid as starting materials.

Methanol for example give hydrogen and trimethylborate:[17] One dominating reaction pattern involves formation of adducts with Lewis bases.

This reaction pattern is rather general and the resulting alkyl borates can be readily derivatized, e.g. to alcohols.

Although early work on hydroboration relied on diborane, it has been replaced by borane dimethylsulfide, which is more safely handled.

[18][19] Although this pyrolysis route is rarely employed, it ushered in a large research theme of borane cluster chemistry.

[20] Diborane is used as a reducing agent roughly complementary to the reactivity of lithium aluminium hydride.

The compound readily reduces carboxylic acids to the corresponding alcohols, whereas ketones react only sluggishly.

[21] Electron diffraction measurements by S. H. Bauer initially appeared to support his proposed structure.

[28] William Nunn Lipscomb Jr. further confirmed the molecular structure of boranes using X-ray crystallography in the 1950s and developed theories to explain their bonding.

Later, he applied the same methods to related problems, including the structure of carboranes, on which he directed the research of future 1981 Nobel Prize winner Roald Hoffmann.

The 1976 Nobel Prize in Chemistry was awarded to Lipscomb "for his studies on the structure of boranes illuminating problems of chemical bonding".

[29] Traditionally, diborane has often been described as electron-deficient, because the 12 valence electrons can only form 6 conventional 2-centre 2-electron bonds, which are insufficient to join all 8 atoms.

[35][36][37] Diborane has been investigated as a precursor to metal boride films[38] and for the p-doping of silicon semiconductors.

Stereo skeletal formula of diborane with all explicit hydrogens added and assorted measurements
Stereo skeletal formula of diborane with all explicit hydrogens added and assorted measurements
Ball and stick model of diborane
Ball and stick model of diborane
NFPA 704 four-colored diamond Health 4: Very short exposure could cause death or major residual injury. E.g. VX gas Flammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propane Instability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxide Special hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
Bonding diagram of diborane (B 2 H 6 ) showing with curved lines a pair of three-center two-electron bonds , each of which consists of a pair of electrons bonding three atoms; two boron atoms and a hydrogen atom in the middle
Borane dimethylsulfide generally functions equivalently to diborane and is easier to use. [ 15 ]